Commercial LPG is primarily a mixture of n-butane and iso-butane. Assuming it to be butane (), what — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

The balanced combustion equation for butane is $C_4H_{10}(g) + \frac{13}{2}O_2(g) \rightarrow 4CO_2(g) + 5H_2O(l)$. The molar mass of butane is $58\text{ g/mol}$. For $1\text{ mole}$ ($58\text{ g}$) of butane, $6.5\text{ moles}$ of $O_2$ are needed. Therefore, for $1000\text{ g}$ of butane, the moles of $O_2$ required = $(1000 / 58) \times 6.5 \approx 112.069\text{ moles}$. At NTP, the volume of $1\text{ mole}$ of gas is $22.4\text{ L}$. Total volume = $112.069 \times 22.4 \approx 2510\text{ L}$.